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(D) The stability of ions in aqueous solution depends on their electronic configuration and hydration energy.For $Ti^{3+}$ $(3d^1)$,$V^{3+}$ $(3d^2)$,

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$Cr^{3+}$

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(D) The stability of ions in aqueous solution depends on their electronic configuration and hydration energy.For $Ti^{3+}$ $(3d^1)$,$V^{3+}$ $(3d^2)$,$Cr^{3+}$ $(3d^3)$,and $Mn^{3+}$ $(3d^4)$,the $Cr^{3+}$ ion is particularly stable due to its half-filled $t_{2g}$ subshell $(t_{2g}^3 e_g^0)$ in an octahedral field.$Mn^{3+}$ is unstable in aqueous solution because it easily reduces to $Mn^{2+}$ $(3d^5)$,which has a stable half-filled $d$-orbital configuration.Therefore,$Cr^{3+}$ is the most stable among the given options in aqueous solution.

Which one of the following ions is the most stable in aqueous solution?
(At. No. $Ti = 22, V = 23, Cr = 24, Mn = 25$)

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Which one of the following ions is the most stable in aqueous solution?(At. No. $Ti = 22, V = 23, Cr = 24, Mn = 25$)